fno lewis structure molecular geometry fno lewis structure molecular geometry

The central atom, carbon, has four valence electrons, and each oxygen atom has six valence electrons. In which of the following pairs of compounds are both members of the pair molecular Not only this, it aids in relaxing muscles and increasing blood flow in the human body. From Figure \(\PageIndex{3}\) we see that with three bonding pairs around the central atom, the molecular geometry of BCl3 is trigonal planar, as shown in Figure \(\PageIndex{2}\). Postby Rajiv Reddy 3K Wed Dec 10, 2014 1:32 pm, Postby BlakeOwens4B Wed Dec 10, 2014 1:41 pm, Users browsing this forum: No registered users and 0 guests. ____________is characterized by a severe reaction to foods containing gluten. A) hydrogen peroxide and ammonia In the following molecules, draw the correct Lewis structure. Predict the geometry of allene (H2C=C=CH2), a compound with narcotic properties that is used to make more complex organic molecules. Thus bonding pairs and lone pairs repel each other electrostatically in the order BPBP < LPBP < LPLP. , Using Standard Molar Entropies), Gibbs Free Energy Concepts and Calculations, Environment, Fossil Fuels, Alternative Fuels, Biological Examples (*DNA Structural Transitions, etc. Both these theories deal with orbitals. The dipole moment of a molecule is therefore the vector sum of the dipole moments of the individual bonds in the molecule. B) CO2 4. E) no correct response. Because lone pairs occupy more space around the central atom than bonding pairs, electrostatic repulsions are more important for lone pairs than for bonding pairs. There are two bonding pairs and one lone pair, so the structure is designated as AX2E. The formal charges, combined with the bent geometry, means that the molecule as a whole is polar, since it has a positive end (nitrogen) and a negative end (the oxygen atoms). There are six electron groups around the Br, five bonding pairs and one lone pair. 11 Uses of Platinum Laboratory, Commercial, and Miscellaneous, CH3Br Lewis Structure, Geometry, Hybridization, and Polarity, Bonding orbital: Here electron density will hold atoms together by attracting the two nuclei, Non-bonding orbital: Here, electrons do not contribute and interact in any form. We can use the VSEPR model to predict the geometry of most polyatomic molecules and ions by focusing only on the number of electron pairs around the central atom, ignoring all other valence electrons present. B There are three electron groups around the central atom, two bonding groups and one lone pair of electrons. H2O molecule also has a bent-shaped structure. Nitrosyl Fluoride or NOF is a nitrosyl compound formed with a covalent bond. Assign an AX m E n designation; then identify the LP-LP, LP-BP, or BP-BP interactions and predict deviations from ideal bond angles. Step 2/2. solon high school swimming; dennison funeral home viola, il; fno lewis structure molecular geometry D There are three nuclei and one lone pair, so the molecular geometry is trigonal pyramidal, in essence a tetrahedron missing a vertex. 4. D) tetrahedral, What is the geometry of the molecular compound formed by the reaction of sulfur with the three-dimensional shape of NO. D With two nuclei about the central atom, the molecular geometry of XeF2 is linear. While this does add up to 0, it is better to have 0 for . Select the correct answer, and write it on the line provided. This leads to sp2 hybridization since we are considering the oxygen atom completing the octet rule. The electronic configuration of Sulfur is 1s 2 2s 2 2p 6 3s 2 3p 4. Save my name, email, and website in this browser for the next time I comment. These structures show the bonding patterns in a compound through the valence electrons. Placing them in the axial positions eliminates 90 LPLP repulsions and minimizes the number of 90 LPBP repulsions. Nitroxyl (HNO); How To Draw Lewis Structure, Molecular Geometry A) Molecular compounds contain two elements, and ionic compounds contain three or Choose the best answer. The theory of hybridization was first proposed by Linus Pauling in 1931. Lewis structures are very useful in predicting the geometry of a molecule or ion. With two bonding pairs and three lone pairs, I3 has a total of five electron pairs and is designated as AX2E3. Because there is one hydrogen and two fluorines, and because of the lone pair of electrons on nitrogen, the molecule is not symmetrical, and the bond dipoles of NHF. The theory of hybridization was first proposed by Linus Pauling in 1931. A combination of VSEPR and a bonding model, such as Lewis electron structures, is necessary to understand the presence of multiple bonds. B) NO2 (6 dots)F--(four dots)O--(6 dots)F. Analysis of an unknown substance showed that it has a high boiling point and is brittle. Gilbert Lewis deduced that the atoms are most stable when the number of valence electrons is equal to eight, this is known as the octet rule. Therefore, the total formal charge on the molecule also becomes zero indicating that the derived Lewis structure is correct. Legal. Both groups around the central atom are bonding pairs (BP). If you have any doubt feel free to ask. With three nuclei and three lone pairs of electrons, the molecular geometry of I3 is linear. ICl4 is designated as AX4E2 and has a total of six electron pairs. Use the VSEPR model to predict the molecular geometry of propyne (H3CCCH), a gas with some anesthetic properties. Required fields are marked *. With no lone pair repulsions, we do not expect any bond angles to deviate from the ideal. Determine the electron group arrangement around the central atom that minimizes repulsions. In this case you want the lowest formal charges for each of the elements. Coming back to NO, we are going to describe its bonding nature in a broad manner here. As the name indicates hybridization refers to the mixing of two or more orbitals such as s, p, d, f, etc. Both (b) and (c) have two 90 LPLP interactions, whereas structure (a) has none. With a double bond on fluorine, oxygen has a formal charge of -1, nitrogen has a formal charge of 0, and fluorine has a formal charge of +1. NO2 Lewis Structure: Drawings, Hybridization, Shape, Charges, Pairs D) more than one correct response 4. By shifting the electron dots from the lateral side towards the center shared by nitrogen and oxygen, we now get nitrogen valency to be 7. document.getElementById( "ak_js_1" ).setAttribute( "value", ( new Date() ).getTime() ); Welcome to Techiescientist.com. following statements is true? The molecular geometry or shape of HNO 2 is bent or V-shaped. N 2 Total \# of Valence Electrons: Lewis Structure: 12. Determine the electron group arrangement around the central atom that minimizes repulsions. The three nuclei in BrF3 determine its molecular structure, which is described as T shaped. NO 2 is, in fact, bent (the bond angle is 136). C) HCN and FNO With two bonding pairs on the central atom and no lone pairs, the molecular geometry of CO2 is linear (Figure \(\PageIndex{3}\)). SF2 Hybridization. B There are four electron groups around oxygen, three bonding pairs and one lone pair. 3. Molecular Geometry - Department of Chemistry The Valence Shell Electron Pair Repulsion (VSEPR) Theory clearly states that electrons inside a molecule tend to arrange themselves in a manner to avoid inter-electronic repulsion. C) NO2 1. D) silicon dioxide, The correct name for the compound H2Te is 4. Molecular geometry, also known as the molecular structure, is the three-dimensional structure or arrangement of atoms in a molecule. This usually occurs due to the difference in electronegativity of combining atoms resulting in the formation of polar bonds. For N to have a near noble gas configuration, we will push towards the double bond formation. Answered: a) FNO Total valence electrons AXE | bartleby In order to maintain uniqueness, all we have to do is calculate the formal charge to see whether all the atoms inside a molecular compound are in their least possible formal charge values. Also indicate the molecular geometry around the central atom the Hybridization around the central atom, and approximate bond angles BH,CN Molecular Geometry around Central Atom hybridi- zation bond angle * HBC BCN NF,OH Molecular Geometry around Central Atom hybridi- zation bond angle A FNO- I * NOH- CH NF Molecular Geometry around Central Atom hybridi- zation bond angle * HCN = * CNF- BrSNCO Molecular Geometry around Central Atom hybridi- zation bond angle BrSN = * SNC *NCO -. 9.2: The VSEPR Model is shared under a CC BY-NC-SA 3.0 license and was authored, remixed, and/or curated by LibreTexts. The valence-shell electron-pair repulsion (VSEPR) model allows us to predict which of the possible structures is actually observed in most cases. Let me know in case you have any queries. In which of the following pairs of triatomic species do both members of the pair have Step 2. 1. It is important to identify the molecular geometry of a compound to illustrate the internal facts about it. . This means that when an atom comes closer to another atom to combine and become a molecule, the electron cloud surrounding each one will repel the other one. Do not add any more atoms. One of the main reasons lies in the emission of nitrogen oxides- NO or nitric oxide. D The PF5 molecule has five nuclei and no lone pairs of electrons, so its molecular geometry is trigonal bipyramidal. Each chlorine contributes seven, and there is a single negative charge. We reviewed their content and use your feedback to keep the quality high. OF2 lewis structure, molecular or electron geometry - Topblogtenz (a) the amino acid serine: (b) urea: (c) pyruvic acid: (d) uracil: (e) carbonic acid: A compound with a molar mass of about 28 g/mol contains 85.7% carbon and 14.3% hydrogen by mass. This concept has a name to it: Valence Shell Electron Pair Repulsion model theory or VSEPR theory. B) LiF is a nonpolar covalent compound and HF is an ionic compound Placing five F atoms around Br while minimizing BPBP and LPBP repulsions gives the following structure: 3. 2. E) no correct response, An angular geometry is associated with molecules in which the central atom has What is the molecular geometry of OCl2? C) H2O When drawing the Lewis structure for nitrosyl fluoride, FNO, why is there a double bond between the nitrogen and oxygen molecules instead of there being a double bond between the nitrogen and fluorine molecules? document.getElementById( "ak_js_1" ).setAttribute( "value", ( new Date() ).getTime() ); Welcome to Techiescientist.com. Step 1: To draw the Lewis structure of NOF we first need to choose a central atom. The central atom, iodine, contributes seven electrons. VSEPR only recognizes groups around the central atom. As clear from the Lewis structure of NOF, three regions of electron density are available around nitrogen atom viz. Molecules with asymmetrical charge distributions have a net dipole moment. As we can see. Required fields are marked *. 3. Step 5. This results in distortion of the molecule, resulting in a bent structure with a bond angle of approximately 110. This approach gives no information about the actual arrangement of atoms in space, however. Take your NO molecule. The four bonds around carbon mean that it must be surrounded by four bonding electron pairs in a configuration similar to AX4. Owing to the charges developed on the molecule due to the electronegativity difference between Oxygen and Fluorine, and also the charge due to the presence of lone pair of the electron the dipole moment of NOF is 1.837 D. The formal charge on the NOF molecule is 0. There are five groups around sulfur, four bonding pairs and one lone pair. fno lewis structure molecular geometry - hansmoeskraal.com Aminooxidanide | H2NO- | CID 160955 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities, safety/hazards/toxicity information, supplier lists, and more. However, we predict a deviation in bond angles because of the presence of the two lone pairs of electrons. Well, they really do and electrons are no exception to this. Thus, all of the valence electrons in PbCl 2 are located on the Cl - ions, and all of the valence electrons in a HCl molecule are shared between the H and Cl atoms.". The molecular geometry can be represented by counting the number of bond and lone pairs in the compound. Draw the Lewis electron structure of the molecule or polyatomic ion. The CoN bond length is 2.1441(18) . Looking at the above structure it is clear that the octet of all the three atoms involved is satisfied and the lone pairs are placed as far apart as possible, indicating this to be the most precise lewis structure for NOF. The total number of electrons around the central atom, S, is eight, which gives four electron pairs. A) H2, F2, and HF are nonpolar covalent molecules ), Administrative Questions and Class Announcements, *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation), *Biological Importance of Buffer Solutions, Equilibrium Constants & Calculating Concentrations, Non-Equilibrium Conditions & The Reaction Quotient, Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions, Reaction Enthalpies (e.g., Using Hesss Law, Bond Enthalpies, Standard Enthalpies of Formation), Heat Capacities, Calorimeters & Calorimetry Calculations, Thermodynamic Systems (Open, Closed, Isolated), Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric), Concepts & Calculations Using First Law of Thermodynamics, Concepts & Calculations Using Second Law of Thermodynamics, Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy, Entropy Changes Due to Changes in Volume and Temperature, Calculating Standard Reaction Entropies (e.g. As nitrogen is the least electronegative element amongst all the three atoms involved it is chosen as the central atom. Two of these electron pairs are bonding pairs and two are lone pairs, so the molecular geometry of \(\ce{H2S}\) is bent (Figure \(\PageIndex{6}\)). So, to comprehend the molecular geometry of NOF, as per the VSEPR theory, we will first have to choose a central atom. NO Lewis Structure, Molecular Geometry, Hybridization, and MO Diagram If you are wondering whether nitric oxide has only harmful effects, be ready to be surprised. Nitrogen has five valence electrons in its outermost shell and Oxygen has six valence electrons. Due to the arrangement of the bonds in molecules that have V-shaped, trigonal pyramidal, seesaw, T-shaped, and square pyramidal geometries, the bond dipole moments cannot cancel one another. As a result, the CO2 molecule has no net dipole moment even though it has a substantial separation of charge. (3) The acronym ORP stands for odor replication process. one lone pair, one double bond, and one single bond. positive and negative, on different atoms of the same molecule. Which of the following statements concerning coordinate covalent bonds is correct? Recognizing similarities to simpler molecules will help you predict the molecular geometries of more complex molecules. Polarity refers to the presence of two opposite charges viz. b. three single bonds, zero double bond, and eight lone pairs. Final answer. From this we can describe the molecular geometry. C) dihydrogen monotelluride 1. A) 2 double bonds and 8 nonbonding electrons. In this case you want the lowest formal charges for each of the elements. PH 3 - use a blue ball for phosphorus when constructing this model Total H of Valence Electrons: Lewis Structure: Bond Angles: 3-D Model Sketch: Molecular Shape(s): Any polar bonds in the molecule? The molecular geometry of PCl5 is trigonal bipyramidal, as shown in Figure \(\PageIndex{3}\). We continue our discussion of structure and bonding by introducing the valence-shell electron-pair repulsion (VSEPR) model (pronounced vesper), which can be used to predict the shapes of many molecules and polyatomic ions. This is known as electron dot structure, another name for Lewis Structure. There are two nuclei about the central atom, so the molecular shape is bent, or V shaped, with an HOH angle that is even less than the HNH angles in NH3, as we would expect because of the presence of two lone pairs of electrons on the central atom rather than one. It has a bent molecular shape: this can be rationalized in the VSEPR model in terms of the lone-pair of electrons located on the N atom. We expect the LPBP interactions to cause the bonding pair angles to deviate significantly from the angles of a perfect tetrahedron. With only bonding pairs, SF6 is designated as AX6. Angular. A step-by-step explanation of how to draw the NOF Lewis Dot Structure (Nitrosyl fluoride).For the NOF structure use the periodic table to find the total numb. All electron groups are bonding pairs (BP). It was first reported in 1930 by Ruff and Krug who prepared it by fluorination of chlorine; this also produced ClF (chlorine monofluoride) and the mixture was separated by distillation.. 3 F 2 + Cl 2 2 ClF 3. View the full answer. B) NH3 1. The two most important resonance structures are shown below. The sulfur atom has six valence electrons and each fluorine has seven valence electrons, so the Lewis electron structure is. The Lewis Structure Generator that we put in your hands here is an excellent tool to obtain structures of more than 400 molecules. The central atom, sulfur, has 6 valence electrons, as does each oxygen atom. With four bonding pairs, the molecular geometry of methane is tetrahedral (Figure \(\PageIndex{3}\)). According to this model, valence electrons in the Lewis structure form groups, which may consist of a single bond, a double bond, a triple bond, a lone pair of electrons, or even a single unpaired electron, which in the VSEPR model is counted as a lone pair. B) Cl2 The next two carbon atoms share a triple bond, and each has an additional single bond. In SO2, we have one BPBP interaction and two LPBP interactions. We also expect a deviation from ideal geometry because a lone pair of electrons occupies more space than a bonding pair. In the O2 molecule, both oxygen atoms have equal electro negativity and both atoms share equal ratios of bonded shared electrons, and the overall molecule turns out to be nonpolar in nature. Schupf Computational Chemistry Lab - Colby College At which trophic level are eagles that consume fish that eat algae? In which of the following molecular compounds are all the bonds single bonds? Here, we have formed this single bond between oxygen and nitrogen but this is not the most suitable form. In the SF2 lewis structure, there is a single bond between sulfur and two fluorine atoms. Which molecule(s) has a net dipole moment? Check out the article I wrote on lewis structure, hybridization, geometry of H2O. The resulting highly exothermic reaction caused a rapid increase in pressure that ruptured the tanks, releasing large amounts of methyl isocyanate that killed approximately 3800 people and wholly or partially disabled about 50,000 others. What is the molecular geometry of FNO? - Answers Preparation, structure, and properties. B) ditellerium monoxide 3. An unpaired electron is present in the Lewis structure for the molecule NO. that contain the prefix di-? In some cases, however, the positions are not equivalent. Lewis electron structures give no information about molecular geometry, the arrangement of bonded atoms in a molecule or polyatomic ion, which is crucial to understanding the chemistry of a molecule. B) Ionic compounds contain oxygen, and molecular compounds do not. Experts are tested by Chegg as specialists in their subject area. Oxygen has six valence electrons and each hydrogen has one valence electron, producing the Lewis electron structure. While hybridization signifies the mixing of atomic orbitals into hybrid orbitals possessing different energy levels, MO theory deals with a linear combination of atomic orbitals to form molecular orbitals. With 18 valence electrons, the Lewis electron structure is shown below. If NO 2 were linear, it would not be polar any more than . . Molecular Weight: 32.022: Computed by PubChem 2.1 (PubChem release 2021.05.07) XLogP3-AA-1.3: Computed by XLogP3 3.0 . Along with the placement of atoms, molecular structure includes various geometrical parameters like bond angle and size. The rainwater is so unusually acidic that it can cause toxicity and poses to be really harmful to life on earth. As shown in Figure \(\PageIndex{2}\), repulsions are minimized by placing the groups in the corners of a tetrahedron with bond angles of 109.5. SF2 Lewis Structure- Key Points. C From B we designate SnCl2 as AX2E. If we look at this sketch, we will find out that the oxygen atom now has eight electrons surrounding it and nitrogen only has five. With three bonding pairs and one lone pair, the structure is designated as AX3E. Explain. Posted at 02:28h in espace o diner saint joseph by who has authority over the sheriff in texas combien de fois le mot pardon dans la bible Likes As we can see in the diagram, we have higher electron density at the non-bonding 2, anti-bonding 1*, and * in Nitrogen. 11. \( \mathrm{PH}_{3} \) - use a blue ball for | Chegg.com NO is a diatomic molecule having unpaired electrons. B) All linear triatomic molecules are nonpolar. The molecular geometry of ClF 3 is approximately T-shaped, with one short bond (1.598 ) and two long bonds (1.698 ). 2003-2023 Chegg Inc. All rights reserved. Notice that this gives a total of five electron pairs. This is not the ultimate solution, since there are debates regarding the hybridization value which is considered to be sometimes sp2 and in other times, sp. contain the same number of atoms per molecule? The central atom, carbon, contributes four valence electrons, and each oxygen atom contributes six. The three lone pairs of electrons have equivalent interactions with the three iodine atoms, so we do not expect any deviations in bonding angles. Therefore, the shape of a molecule is determined by the number of lone pairs present as well as the extent of electronic repulsion present in the molecule. Molecular structure describes the location of the atoms, not the electrons. The molecular geometry can be described as a trigonal planar arrangement with one vertex missing. This designation has a total of four electron pairs, three X and one E. We expect the LPBP interactions to cause the bonding pair angles to deviate significantly from the angles of a perfect tetrahedron. not. National Center for Biotechnology Information . The lewis structure of OF2 is very easy to . D) hydrogen monotelluride, Which of the following statements concerning differences between ionic and molecular D) more than one correct response Molecules with polar covalent bonds can have a dipole moment, an asymmetrical distribution of charge that results in a tendency for molecules to align themselves in an applied electric field. Because the carbon atom on the left is bonded to four other atoms, we know that it is approximately tetrahedral. Draw the Lewis electron structure of the molecule or polyatomic ion. Keep in mind, however, that the VSEPR model, like any model, is a limited representation of reality; the model provides no information about bond lengths or the presence of multiple bonds. In 1984, large quantities of Sevin were accidentally released in Bhopal, India, when water leaked into storage tanks. The strength of the bonds and the reactivity of the molecules result in a wide varied range of properties be it hardness, boiling point, or conductivity. Although a molecule like CHCl3 is best described as tetrahedral, the atoms bonded to carbon are not identical. We see from Figure \(\PageIndex{2}\) that the geometry that minimizes repulsions is octahedral. CHEM 1P91 Question 10. A) F, Br, As Lewis structure is 2D and molecular geometry is the 3d version. Smith, Michael Abbott. The central N-atom is sp 2 hybridized in HNO 2. SF2 molecule is polar in nature. USA Distributor of MCM Equipment fno lewis structure molecular geometry I am Savitri,a science enthusiast with a passion to answer all the questions of the universe. (2) The molecule nitric oxide is naturally present in the human body. The lewis structure of OF2 contains 8 lone pairs (2 lone pairs on oxygen (O) atom and 3 lone pairs on each fluorine (F) atom). The central atom, boron, contributes three valence electrons, and each chlorine atom contributes seven valence electrons. Each group around the central atom is designated as a bonding pair (BP) or lone (nonbonding) pair (LP). In the following molecules, draw the correct Lewis structure. For example, the sp3 orbital indicates that one s and 3 p orbitals were mixed for its formation. Owing to the presence of an unpaired electron, it acts as a free radical and is reactive in nature. 1. NOF Lewis Structure, Geometry, Hybridization, and Polarity E) no correct response, Which of the following tetrahedral molecules is polar? E) no correct response, Which of the following statements concerning molecular polarity is correct? D) more than one correct response In this article, we will study the lewis structure of NOF, its hybridization, polarity, and geometry. A) SCl2 and K2O All positions are chemically equivalent, so all electronic interactions are equivalent. ), Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams, Work, Gibbs Free Energy, Cell (Redox) Potentials, Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH), Interesting Applications: Rechargeable Batteries (Cell Phones, Notebooks, Cars), Fuel Cells (Space Shuttle), Photovoltaic Cells (Solar Panels), Electrolysis, Rust, Kinetics vs. Thermodynamics Controlling a Reaction, Method of Initial Rates (To Determine n and k), Arrhenius Equation, Activation Energies, Catalysts, Chem 14B Uploaded Files (Worksheets, etc. The Lewis electron structure is. Repulsions are minimized by directing each hydrogen atom and the lone pair to the corners of a tetrahedron. Groups are positioned around the central atom in a way that produces the molecular structure with the lowest energy, as illustrated in Figures \(\PageIndex{1}\) and \(\PageIndex{2}\). It is Linear. sc < tun x = | Kotcthaltoth Gtntementmlst thc ren Ineeule Dneed Rule (noscn ficon mlenu Oreailea &escnDticn 5C Cctt mofmarinn autot Sotettari 00 0-0 Ded Senci Aule Fefm D+0 Ee D Hollnli 0,6 0-0 It is based on the assumption that pairs of electrons occupy space, and the lowest-energy structure is the one that minimizes electron pairelectron pair repulsions. The axial and equatorial positions are not chemically equivalent, as we will see in our next example. SF2 molecular geometry is bent. This is because a multiple bond has a higher electron density than a single bond, so its electrons occupy more space than those of a single bond. We designate SF4 as AX4E; it has a total of five electron pairs. This VESPR procedure is summarized as follows: We will illustrate the use of this procedure with several examples, beginning with atoms with two electron groups. tastier star jellies cookie run kingdom. We will work with and here, so before we go direct, heres just a quick view: Sigma orbitals are found to be symmetric across the bond axis and Pi orbitals are found along a nodal plane with the bond axis. Draw the Lewis. So, all these negative charges together point towards the sole fact that they are going to repel each other based on their like nature. This is because the nature of chemical bonding between atoms determines the molecular shape of a molecule. A) germanium tetrabromide For N: Total number of the valence electrons in Free State = 5, Putting these values in above formula, Formal Charge = 5 [ 2 6/2] = 0, For O: Total number of valence electron in Free State = 6, Putting these values in above formula, Formal Charge = 6 [ 4 4/2] = 0, Similarly for F: Total number of valence electron in Free State = 7, Putting these values in above formula, Formal Charge = 7 [ 6 2/2] = 0. Step 2: Now counting the number of valence electrons in the molecule: For Nitrogen (Group 15 element), number of valence electron = 5, For Oxygen (Group 16 element), number of valence electron = 6, For Fluorine (Group 17 element), number of valence electron = 7, Now counting total number of valence electron= 5 + 6 + 7.